Hi, I was able to do the 'simpler' titrations that we were given, but I keep doing this one but I don't get the correct answer (I don't think I do at least)... Could anyone explain where I went wrong/why? Thanks!
"A 1.575g sample of ethanedioic acid crystals, H2C2O4.nH20 was dissolved in water and made up 250cm^3. One mole of the acid reacts with two moles of NaOH. In a titration, 25.0cm^3 of this solution of acid reacted with exactly 15.6cm^3 of 0.16moldm^-3 NaOH. Calculate the value of n".
I realised that you just do a 'normal titration' and you either multiply both volumes by 10, or divide the g by 10.
So I did: 15.6cm^3/1000 = 0.0156dm^3
0.16 mol dm^-3*0.0156=0.002496 moles.
1 mole of acid : 2 moles of NaOH.
So 0.002496/2=0.001248moles
then you use the g/mol formula, so divide the 'g' by 1.575 by 10 to get 0.1575. So 0.1575/0.001248=126
And then the RFM of H2C2O4= 90. So 126-90=46. Then you divide by RFM of water (18) to get n. So 46/18 = 2.5. So n = 2.5? But loads of other people say it's like 50? :s